Select correct statement :

Options

A. The decomposition of an oxide into oxygen and metal vapour entropy increases
B. Decomposition of an oxide is an endothermic change
C. The make `Delta G^(@)` negative, temperature should be high enough so that `T Delta S^(@) gt Delta H^(@)`
D. All are correct statements

Explanation

To solve the question, we need to analyze each statement provided in the question regarding the decomposition of an oxide into oxygen and metal vapor.

### Step-by-Step Solution:

1. **Statement A: Decomposition of an oxide into oxygen and metal vapor increases entropy.**
- When an oxide decomposes, it produces a solid metal and a gas (oxygen). The formation of gas from a solid increases the randomness of the system, which means that entropy increases.
- **Conclusion:** This statement is **correct**.

2. **Statement B: Decomposition of an oxide is an endothermic change.**
- An endothermic reaction is one that absorbs heat from the surroundings. The decomposition of many metal oxides requires energy input (heat) to break the bonds in the oxide, indicating that it is endothermic.
- **Conclusion:** This statement is **correct**.

3. **Statement C: To make ΔG negative, the temperature should be high enough so that TΔS is greater than ΔH.**
- The Gibbs free energy change (ΔG) is given by the equation ΔG = ΔH - TΔS. For a reaction to be spontaneous (ΔG < 0), it is necessary that TΔS > ΔH. This means that at high temperatures, the entropy term can outweigh the enthalpy term, making ΔG negative.
- **Conclusion:** This statement is **correct**.

4. **Statement D: All are correct.**
- Since all previous statements (A, B, and C) have been found to be correct, this statement must also be correct.
- **Conclusion:** This statement is **correct**.

### Final Answer:
All statements (A, B, C, and D) are correct.

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